Question

Two sparingly soluble salts $AX$ and $BX _{2}$ have their solubility product constants equal. Which of the following is incorrect ?

• A. Solubility of $AX$ is less than solubility of $BX _{2}$
• B. If $S _{1}$ and $S _{2}$ are molar solubility of $AX$ and $BX _{2}$ then $S _{1}=2\left( S _{2}\right)^{2 / 3}$
• C. If $X$ is a conjugate base of a weak acid, addition of $HNO _{3}$ will increase solubility of both $AX$ and $BX _{2}$
• D. Increasing the temperature, increases the solubility of both $AX$ and $BX _{2}$

Answer 1

Answer: (B)

$Ksp _{1}= s ^{2}$
$Ksp _{2}=4 s ^{'3}$
$s ^{2}=4 s ^{'3}$